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Stoichiometry  Objectives  Describe a method for determining which of two reactants is a limiting reactant  Calculate the amount in moles or mass in grams of a product, given the amounts in moles or masses in grams of two reactants, one of which is in excess  Distinguish between theoretical yield, actual yield, and percentage yield  Calculate percentage yield, given the actual yield and quantity of a reactant

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Stoichiometry  Limiting Reactions  The limiting reactant is the reactant that limits the amount of the other reactant that can combine and the amount of product that can form in a chemical reaction  The excess reactant is the substance that is not used up completely in a reaction

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Stoichiometry  Percentage Yield  The theoretical yield is the maximum amount of product that can be produced from a given amount of reactant  The actual yield of a product is the measured amount of that product obtained from a reaction  The percentage yield is the ratio of the actual yield to the theoretical yield, multiplied by 100

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In the commercial production of the element arsenic, arsenic(III) oxide is heated with carbon, which reduces the oxide to the metal according to the following equation: 2As 2 O 3 + 3C  3CO 2 +4As If 8.87 g of As 2 O 3 is used in the reaction and 5.33 g of As is produced, what is the percentage yield? Stoichiometry

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A process by which zirconium metal can be produced from the mineral zirconium(IV) orthosilicate, ZrSiO 4, starts by reacting it with chlorine gas to form zirconium(IV) chloride. ZrSiO 4 + 2Cl 2  ZrCl 4 + SiO 2 + O 2 What mass of ZrCl 4 can be produced if 862 g of ZrSiO 4 and 950. g of Cl 2 are available? Stoichiometry

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Hydrogen is generated by passing hot steam over iron, which oxidizes to form Fe 3 O 4, in the following equation. 3Fe(s) + 4H 2 O(g)  4H 2 (g) + Fe 3 O 4 (s) If 625 g of Fe 3 O 4 is produced in the reaction, how many moles of hydrogen are produced at the same time? Stoichiometry